(B) The rate law for the reaction is given by: $r = k[A]^1[B]^2$. If the concentration of $B$ is increased $3$ times,the new concentration becomes $[B

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(B) The rate law for the reaction is given by: $r = k[A]^1[B]^2$. If the concentration of $B$ is increased $3$ times,the new concentration becomes $[B'] = 3[B]$. The new rate is $r_{new} = k[A][3B]^2$. $r_{new} = k[A] \times 9[B]^2 = 9 \times (k[A][B]^2)$. $r_{new} = 9r$. Therefore,the reaction rate increases $9$ times.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

MHT CET 2021 All MHT CET

A
Rate increases $6$ times
B
Rate increases $9$ times
C
Rate increases $2$ times
D
Rate increases $3$ times

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Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.

DifficultAIIMS 2011

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The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$
Experiment $[Cl_2] \ (M)$ $[NO] \ (M)$ Rate $(mol \ L^{-1} \sec^{-1})$
$I$ $0.05$ $0.05$ $1 \times 10^{-3}$
$II$ $0.15$ $0.05$ $3 \times 10^{-3}$
$III$ $0.05$ $0.15$ $9 \times 10^{-3}$

The rate law for the reaction is:

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The reaction $2FeCl_3 + SnCl_2 \rightarrow 2FeCl_2 + SnCl_4$ is an example of a .......

Easy

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The rate of the reaction,$CH_3COOC_2H_5 + NaOH \longrightarrow CH_3COONa + C_2H_5OH$ is given by the equation,$\text{rate} = k[CH_3COOC_2H_5][NaOH]$. If concentration is expressed in $mol \ L^{-1}$,the unit of $k$ is

EasyKCET 2022

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The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:

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Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

Similar Questions

Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.Reason : The rate of the reaction does not depend upon the concentration of $C$.

The given data are for the reaction:$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$Experiment$[Cl_2] \ (M)$$[NO] \ (M)$Rate $(mol \ L^{-1} \sec^{-1})$$I$$0.05$$0.05$$1 \times 10^{-3}$$II$$0.15$$0.05$$3 \times 10^{-3}$$III$$0.05$$0.15$$9 \times 10^{-3}$The rate law for the reaction is:

The reaction $2FeCl_3 + SnCl_2 \rightarrow 2FeCl_2 + SnCl_4$ is an example of a .......

The rate of the reaction,$CH_3COOC_2H_5 + NaOH \longrightarrow CH_3COONa + C_2H_5OH$ is given by the equation,$\text{rate} = k[CH_3COOC_2H_5][NaOH]$. If concentration is expressed in $mol \ L^{-1}$,the unit of $k$ is

The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:

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Assertion : The kinetics of the reaction $mA + nB + pC \to m'X + n'Y + p'Z$ obey the rate expression as $\frac{dX}{dt} = k[A]^m[B]^n$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.